Ammonium ion reacts slowly with nitrite ion: NH4+ (aq) + NO2-(aq)-> N2(g) + 2H2O(1) Rate data for this reaction, measured at a certain temperature, are shown in the attached table. Use your rate law, and the rate and concentrations for any of the experiments, to calculate the rate constant (k) for the reaction in /Ms. Type your response Expt. [NH4+] (M) [NO₂ ] (M) Rate (M s-1) 1 0.150 0.220 7.00 x 10-6 2 0.600 0.220 2.80 x 10-5 3 0.600 0.110 1.40 x 10-5

Help with the question on the right Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, find the rate law. 0–H (RCOOH), M [R'OHJ, M (HAJ, M Initial Rate, M-min"' - R-C+ k2 R С—0—Н + HA A- 0.35 0.35 0.50 4.60 0.50 0.62 0.35 0.35 8.14 0.81 0.50 10.6 0.35 0.50 0.75 0–H 9.84 Group 1 0–H 0–H k3 Rate = k[RCOOH][R'OH] R-Ć+ A- R 0–H R—С—0—Н + Rate = k[RCOOH][R'OH][HA] k4 0–H R-ó+ A- Group 2 Rate = k[RCOOR']/{[RCOOH][R'OH]} H Rate = k[R'OH] 0–H Rate = k[RCOOH] k5 R- C-0–R' R-C-0–H + H,о + НА R-o+ A- Group 3 Step 2 or Step 3 O Step 1 or Step 2 Step 1 Step 3 Step 2 Step 1

rate = k [A]1 [B]1  (k = 5.8 M-1∙s-1) Using the above rate law, deduce what volumes of the A and B solutions, and water would need to be combined to achieve a color change at the 90 second mark (you can disregard the need for the B-dilution solution).  You must annotate your calculations (tell me why you are doing what you are doing).  Remember that the total volume will need to be 20 mL, and that the starting concentrations of the A is 0.0090 M,  and B is 0.0050 M.